3.2 Gas Laws Unit Assessment

Learning Target 3.2.1: I can convert between various units of pressure, temperature, and volume.

Goal 3.2.1.a I can explain how pressure and temperature are related to the Kinetic Molecular Theory

Goal 3.2.1.b I understand what pressure is and I can convert between different units of pressure.

Goal 3.2.1.c I understand what temperature is and I can convert between different units of temperature.

Goal 3.2.1.d I understand what volume is and I can convert between different units of volume.

Learning Target 3.2.2: I can explain the relationships between volume of a gas, its temperature and its pressure using Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, and the Combined Gas Law and how changing one variable affects the others.

Goal 3.2.2.a I can identify a graph of two variables as directly proportional or inversely proportional.

Goal 3.2.2.b I can demonstrate that under constant temperature, if you increase the pressure you will decrease the volume.

Goal 3.2.2.c I can calculate the change in volume or pressure of a gas in a closed system if I know the change in pressure or volume at a constant temperature using

P1V1 = P2V2 (Boyle’s Law)

Goal 3.2.2.d I can demonstrate that under constant pressure, if you increase the temperature you will increase the volume.

Goal 3.2.2.e I can calculate the change in volume or temperature of a gas in a closed system if I know the change in temperature or volume at a constant pressure using V1/T1 = V2/T2 (Charles’s Law)

Goal 3.2.2.f I can calculate the change in volume or pressure of a gas in a closed system if I know the change in pressure or temperature at a constant volume using P1/T1 = P2/T2 (Gay-Lussac’s Law)

Goal 3.2.2.g I can calculate the change in temperature, volume or pressure of a gas in a closed system if I know the change in the other variables using P1V1/T1 = P2V2/T2 (Combined Gas Law)

Goal 3.2.2.h I can calculate the change in volume or number of moles of a gas in a closed system if I know the change in volume or number of moles at a constant temperature and pressure using V1/n1 = V2/n2 (Avogadro’s Law)

Learning Target 3.2.3: I can explain the Ideal Gas Law and how it relates to kinetic molecular theory.

Goal 3.2.3.a I can describe how the Kinetic Molecular Theory relates to an Ideal Gas.

Goal 3.2.3.b I can identify the units of Standard Temperature and Pressure that will be used in calculations.

Goal 3.2.3.c I can calculate one unknown from PV=nRT if I know the other three variable values.

MNPCC 3.2 Gas Laws Unit Assessment

Multiple Choice

Identify the choice that best completes the statement or answers the question.

1. What does the constant bombardment of gas molecules against the inside walls of a container produce?

a. temperature

b. density

c. pressure

d. diffusion

2. If force is held constant as surface area increases, pressure

a. remains constant.

b. decreases.

c. increases.

d. increases or decreases, depending on the volume change.

3. According to the kinetic-molecular theory, particles of matter

a. have different shapes

b. are always fluid

c. are in constant motion.

d. have different colors.

4. The kinetic-molecular theory explains the properties of solids, liquids, and gases in terms of the forces that act between the particles and

a. gravitational forces.

b. the energy of the particles.

c. diffusion.

d. the mass of the particles.

5. Unlike in an ideal gas, in a real gas

a. the particles cannot diffuse.

b. the particles exert attractive forces on each other.

c. all particles move in the same direction.

d. all particles have the same kinetic energy.

6. Why does a can collapse when a vacuum pump removes air from the can?

a. The atmosphere exerts pressure on the inside of the can and crushes it.

b. The vacuum pump creates a force that crushes the can.

c. The inside and outside forces balance out and crush the can.

d. The unbalanced outside force from atmospheric pressure crushes the can.

7. A pressure of 730 mm Hg equals

a. 730 torr.

b. 1 torr.

c. 1 pascal.

d. 730 pascal.

8. Convert the pressure 0.50 atm to mm Hg.

a. 101.325 mm Hg

b. 380mmHg

c. 760 mmHg

d. 1520 mmHg

9. Convert the pressure 2.20 atm to kPa.

a. 0.0217 kPa .

b. 223 kPa

c. 760 kPa

d. 1000 kPa

10. Standard temperature is exactly

a. 0 K.

b. 0°C

c. 100°C.

d. 273°C.

11. Standard pressure is exactly

a. 1 atm.

b. 760 atm.

c. 101.325 atm.

d. 101 atm.

12. The volume of a gas is 800.0 mL when the pressure is 1.00 atm. At the same temperature, what is the pressure at which the volume of the gas is 2.0 L?

a. 0.25 atm

b. 0.40 atm

c. 1.60 atm

d. 2.5 atm

13. The volume of a gas is 4.0 L when the temperature is 5.0°C. If the temperature is increased to 10.0°C without changing the pressure, what is the new volume?

a. 2.0 L

b. 3.9 L

c. 4.1 L

d. 8.0 L

14. The volume of a sample of oxygen is 400.0 mL when the pressure is 1.00 atm and the temperature is 27.0°C. At what temperature is the volume 1.00 L and the pressure 0.500 atm?

a. 25.0°C

b. 33.8°C

c. 0.50 K

d. 375 K

15. In the equation H2 + Cl2 → 2 HCl, one volume of hydrogen yields how many volumes of hydrogen chloride.

a. 1

b. 2

c. 3

d. 4

16. If 0.5 L of O2(g) reacts with H2 to produce 1 L of H2O(g) , what is the volume of H2O(g) obtained from 1 L of O2(g)?

a. 0.5L

b. 1.5 L

c. 2L

d. 2.5L

17. Equal volumes of diatomic gases under the same conditions of temperature and pressure contain the same number of

a. protons.

b. ions.         

c. molecules.

d. electrons.

18. According to Avogadro's law, 1 L of H2 (g) and 1 L of O2(g) at the same temperature and pressure

a. have the same mass.

b. have unequal volumes.

c. contain 1 mol of gas each.

d. contain equal numbers of molecules.

19. The standard molar volume of a gas is all of the following except

a. the volume occupied by 1 mol of a gas at STP.

b. equal for all gases under the same conditions.

c. 22.4 L at STP.

d. dependent upon the size of the molecules.

20. What is the volume occupied by 1 mol of oxygen at STP?

a. 11.2 L

b. 16.0 L

c. 22.4 L

d. 32.0 L

21. What is the volume occupied by 1 mol of water vapor at STP?

a. 11.2 L

b. 18.0 L

c. 22.4 L

d. 33.6 L

22. All of the following equations are statements of the ideal gas law except

a.

b.

c.

d.

23.

This is a graph of volume readings collected when the temperature changes from 270K to 340K. This graph shows that temperature and volume are

a. directly proportional

b. inversely proportional

24. Boyle’s Law shows that pressure and volume are inversely proportional. The slope of the line graphing pressure vs volume would have

a. positive slope

b. zero slope

c. negative slope

d. first positive, then negative slope